1. Write the rate expression for the following reaction.2N2O5(g) → 4

1.	1. Write the rate expression for the following reaction.2N2O5(g) → 4NO2(g) + O2(g)2. For a hypothetical reaction, aX + bY → Products, the rate law is given as \(\frac{dx}{dt}=\) k[X]2[Y]1/2. What happens to the rate of the reaction whenThe concentration of ‘X’ is doubled keeping that of ‘Y’ constant.The concentration of both ‘Y’ is doubled keeping that of ‘X’ constant.
Answer» 1. Rate expression : Rate = \(-\frac{1}{2}\,\frac{d[N_2O_5]}{dt}=\)\(+\frac{1}{4}\,\frac{d[NO_2]}{dt}= + \frac{d[O_2]}{dt}\) 2. Increases by 4 times Increases by \(\sqrt2\) times.

1. Write the rate expression for the following reaction.2N2O5(g) → 4NO2(g) + O2(g)2. For a hypothetical reaction, aX + bY → Products, the rate law is given as \(\frac{dx}{dt}=\) k[X]2[Y]1/2. What happens to the rate of the reaction whenThe concentration of ‘X’ is doubled keeping that of ‘Y’ constant.The concentration of both ‘Y’ is doubled keeping that of ‘X’ constant.

Answer»

1. Rate expression :

Rate = \(-\frac{1}{2}\,\frac{d[N_2O_5]}{dt}=\)\(+\frac{1}{4}\,\frac{d[NO_2]}{dt}= + \frac{d[O_2]}{dt}\)

Increases by 4 times
Increases by \(\sqrt2\) times.

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